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KOH + NO2 + KClO = H2O + KCl + KNO3

Input interpretation

KOH potassium hydroxide + NO_2 nitrogen dioxide + KClO ⟶ H_2O water + KCl potassium chloride + KNO_3 potassium nitrate
KOH potassium hydroxide + NO_2 nitrogen dioxide + KClO ⟶ H_2O water + KCl potassium chloride + KNO_3 potassium nitrate

Balanced equation

Balance the chemical equation algebraically: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 NO_2 + c_3 KClO ⟶ c_4 H_2O + c_5 KCl + c_6 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, N and Cl: H: | c_1 = 2 c_4 K: | c_1 + c_3 = c_5 + c_6 O: | c_1 + 2 c_2 + c_3 = c_4 + 3 c_6 N: | c_2 = c_6 Cl: | c_3 = c_5 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3
Balance the chemical equation algebraically: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 NO_2 + c_3 KClO ⟶ c_4 H_2O + c_5 KCl + c_6 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, N and Cl: H: | c_1 = 2 c_4 K: | c_1 + c_3 = c_5 + c_6 O: | c_1 + 2 c_2 + c_3 = c_4 + 3 c_6 N: | c_2 = c_6 Cl: | c_3 = c_5 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3

Structures

+ + KClO ⟶ + +
+ + KClO ⟶ + +

Names

potassium hydroxide + nitrogen dioxide + KClO ⟶ water + potassium chloride + potassium nitrate
potassium hydroxide + nitrogen dioxide + KClO ⟶ water + potassium chloride + potassium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 2 | -2 NO_2 | 2 | -2 KClO | 1 | -1 H_2O | 1 | 1 KCl | 1 | 1 KNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) NO_2 | 2 | -2 | ([NO2])^(-2) KClO | 1 | -1 | ([KClO])^(-1) H_2O | 1 | 1 | [H2O] KCl | 1 | 1 | [KCl] KNO_3 | 2 | 2 | ([KNO3])^2 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([KOH])^(-2) ([NO2])^(-2) ([KClO])^(-1) [H2O] [KCl] ([KNO3])^2 = ([H2O] [KCl] ([KNO3])^2)/(([KOH])^2 ([NO2])^2 [KClO])
Construct the equilibrium constant, K, expression for: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 2 | -2 NO_2 | 2 | -2 KClO | 1 | -1 H_2O | 1 | 1 KCl | 1 | 1 KNO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) NO_2 | 2 | -2 | ([NO2])^(-2) KClO | 1 | -1 | ([KClO])^(-1) H_2O | 1 | 1 | [H2O] KCl | 1 | 1 | [KCl] KNO_3 | 2 | 2 | ([KNO3])^2 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([KOH])^(-2) ([NO2])^(-2) ([KClO])^(-1) [H2O] [KCl] ([KNO3])^2 = ([H2O] [KCl] ([KNO3])^2)/(([KOH])^2 ([NO2])^2 [KClO])

Rate of reaction

Construct the rate of reaction expression for: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 2 | -2 NO_2 | 2 | -2 KClO | 1 | -1 H_2O | 1 | 1 KCl | 1 | 1 KNO_3 | 2 | 2 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) NO_2 | 2 | -2 | -1/2 (Δ[NO2])/(Δt) KClO | 1 | -1 | -(Δ[KClO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[KOH])/(Δt) = -1/2 (Δ[NO2])/(Δt) = -(Δ[KClO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + NO_2 + KClO ⟶ H_2O + KCl + KNO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 KOH + 2 NO_2 + KClO ⟶ H_2O + KCl + 2 KNO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 2 | -2 NO_2 | 2 | -2 KClO | 1 | -1 H_2O | 1 | 1 KCl | 1 | 1 KNO_3 | 2 | 2 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) NO_2 | 2 | -2 | -1/2 (Δ[NO2])/(Δt) KClO | 1 | -1 | -(Δ[KClO])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[KOH])/(Δt) = -1/2 (Δ[NO2])/(Δt) = -(Δ[KClO])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KCl])/(Δt) = 1/2 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | nitrogen dioxide | KClO | water | potassium chloride | potassium nitrate formula | KOH | NO_2 | KClO | H_2O | KCl | KNO_3 Hill formula | HKO | NO_2 | ClKO | H_2O | ClK | KNO_3 name | potassium hydroxide | nitrogen dioxide | | water | potassium chloride | potassium nitrate IUPAC name | potassium hydroxide | Nitrogen dioxide | | water | potassium chloride | potassium nitrate
| potassium hydroxide | nitrogen dioxide | KClO | water | potassium chloride | potassium nitrate formula | KOH | NO_2 | KClO | H_2O | KCl | KNO_3 Hill formula | HKO | NO_2 | ClKO | H_2O | ClK | KNO_3 name | potassium hydroxide | nitrogen dioxide | | water | potassium chloride | potassium nitrate IUPAC name | potassium hydroxide | Nitrogen dioxide | | water | potassium chloride | potassium nitrate

Substance properties

| potassium hydroxide | nitrogen dioxide | KClO | water | potassium chloride | potassium nitrate molar mass | 56.105 g/mol | 46.005 g/mol | 90.55 g/mol | 18.015 g/mol | 74.55 g/mol | 101.1 g/mol phase | solid (at STP) | gas (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | -11 °C | | 0 °C | 770 °C | 334 °C boiling point | 1327 °C | 21 °C | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 1.98 g/cm^3 | solubility in water | soluble | reacts | | | soluble | soluble surface tension | | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 4.02×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless | odorless
| potassium hydroxide | nitrogen dioxide | KClO | water | potassium chloride | potassium nitrate molar mass | 56.105 g/mol | 46.005 g/mol | 90.55 g/mol | 18.015 g/mol | 74.55 g/mol | 101.1 g/mol phase | solid (at STP) | gas (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 406 °C | -11 °C | | 0 °C | 770 °C | 334 °C boiling point | 1327 °C | 21 °C | | 99.9839 °C | 1420 °C | density | 2.044 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 1.98 g/cm^3 | solubility in water | soluble | reacts | | | soluble | soluble surface tension | | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | 4.02×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | odorless | odorless

Units

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